chapter-19 lecture-4

chapter-19 lecture-4 - Review: Acid-Base Titration...

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Review: Acid-Base Titration itration solution of nown oncentration is added gradually Titration a solution of known concentration is added gradually to another solution of unknown concentration until the chemical reaction between the two solutions is complete. Equivalence point – the point at which the reaction is complete (for example, 1 mol NaOH reacted with 1 mol HCl ) Endpoint of the titration: the point at which the indicator changes color If the indicator is chosen correctly the end point is very close to the quivalence point Slowly add base equivalence point to unknown acid UNTIL The indicator 19-26 changes color
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Curve for a weak base-strong acid titration. HCl (titrant) Be careful in choosing the indicator H NH 3 A weak base 19-27
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Finding the Equivalence Point alculation method) (calculation method) • Strong Acid vs. Strong Base 00 % ionized! pH = 7 – 100 % ionized! pH = 7 • Weak Acid titrated by Strong Base – Acid is neutralized; Need K b for conjugate base equilibrium eak Base titrated by Strong cid • Weak Base titrated by Strong Acid – Base is neutralized; Need K a for conjugate acid equilibrium • Weak Acid vs. Weak Base – Depends on the strength of both; could be onjugate acid conjugate base or pH 7 19-28 conjugate acid, conjugate base, or pH 7
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Curve for the titration of a weak polyprotic acid.
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This note was uploaded on 07/31/2010 for the course CHEM CHEM 01C taught by Professor Unknown during the Spring '10 term at UC Riverside.

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chapter-19 lecture-4 - Review: Acid-Base Titration...

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